Q
QuestionChemistry

Draw the Lewis structure for COCl^2, including lone pairs. What is the molecular shape of COCl^2? The C - Cl bond in COCl^2 is polar or nonpolar? What is the Cl - C - Cl bond angle? The molecule COCl^2 is polar or nonpolar?

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Answer

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Step 1:
: Draw the Lewis structure for COCl^2.

To draw the Lewis structure, first count the total number of valence electrons for the molecule. Carbon (C) is in the 4th group, so it has 4 valence electrons. Oxygen (O) is in the 6th group, so it has 6 valence electrons. Chlorine (Cl) is also in the 7th group, so it has 7 valence electrons. The molecule contains one carbon atom, one oxygen atom, and two chlorine atoms, so the total number of valence electrons is: \text{Total valence electrons} = 4 \text{(C)} + 6 \text{(O)} + 7 \text{(Cl)} + 7 \text{(Cl)} = 24 Now, subtract the number of electrons used to form bonds. In this case, there are two single bonds (each using 2 electrons) between carbon and chlorine atoms, and one double bond (using 4 electrons) between carbon and oxygen atoms. Therefore, the number of electrons used to form bonds is: \text{Bonding electrons} = 2 \text{(C-Cl bonds)} + 4 \text{(C=O bond)} = 8 The remaining electrons are non-bonding electrons (lone pairs). In this case, we have: \text{Lone pairs} = \text{Total valence electrons} - \text{Bonding electrons} = 24 - 8 = 16 Distribute the valence electrons around the molecule, ensuring that each atom has 8 electrons in its outer shell. The resulting Lewis structure for COCl^2 is: \mathrm{O} : \underbrace{\overbrace{\boxed{\cdot \mathrm{C} \cdot}}^{\text{double bond}} : \mathrm{Cl}}_{\text{single bond}} : \mathrm{Cl}

Step 2:
: Determine the molecular shape of COCl^2.

The molecular shape is determined by the central atom's bonded and non-bonded electron pairs. In this case, the central atom is carbon, which has two bonded chlorine atoms and one double-bonded oxygen atom. The electron pairs around the central carbon atom form a linear geometry. Therefore, the molecular shape of COCl^2 is linear.

Step 3:
: Determine if the C - Cl bond in COCl^2 is polar or nonpolar.

The C - Cl bond is polar because chlorine is more electronegative than carbon.

Step 4:
: Determine the Cl - C - Cl bond angle.

Since the molecular shape of COCl^2 is linear, the bond angle between the two chlorine atoms is 180 degrees.

Step 5:
: Determine if the molecule COCl^2 is polar or nonpolar.

The molecule is polar because the C - Cl bond is polar and the bond angle is 180 degrees, which does not allow the dipole moments to cancel out.

Final Answer

1. The Lewis structure for COCl^2 is: \mathrm{O} : \underbrace{\overbrace{\boxed{\cdot \mathrm{C} \cdot}}^{\text{double bond}} : \mathrm{Cl}}_{\text{single bond}} : \mathrm{Cl} 2. The molecular shape of COCl^2 is linear. 3. The C - Cl bond in COCl^2 is polar. 4. The Cl - C - Cl bond angle is 180 degrees. 5. The molecule COCl^2 is polar.

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Q
QuestionChemistry

Answer

Full Solution Locked

Step 1:
: Draw the Lewis structure for COCl^2.

Step 2:
: Determine the molecular shape of COCl^2.

Step 3:
: Determine if the C - Cl bond in COCl^2 is polar or nonpolar.

Step 4:
: Determine the Cl - C - Cl bond angle.

Step 5:
: Determine if the molecule COCl^2 is polar or nonpolar.

Final Answer

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QQuestionChemistry

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Full Solution Locked

Step 1:: Draw the Lewis structure for COCl^2.

Step 2:: Determine the molecular shape of COCl^2.

Step 3:: Determine if the C - Cl bond in COCl^2 is polar or nonpolar.

Step 4:: Determine the Cl - C - Cl bond angle.

Step 5:: Determine if the molecule COCl^2 is polar or nonpolar.

Final Answer

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Related Questions

Q
QuestionChemistry

Answer

Step 1:
: Draw the Lewis structure for COCl^2.

Step 2:
: Determine the molecular shape of COCl^2.

Step 3:
: Determine if the C - Cl bond in COCl^2 is polar or nonpolar.

Step 4:
: Determine the Cl - C - Cl bond angle.

Step 5:
: Determine if the molecule COCl^2 is polar or nonpolar.